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The [H+] of 0.1 M acetic acid solution is 1.33 × 10–3. The pH of the solution (correct to two decimal places) is _______ .
    Correct answer is between `2.86,2.89`. Can you explain this answer?
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    The [H+] of 0.1 M acetic acid solution is 1.33 × 10–3. The pH of the s...
    Calculation of pH of Acetic Acid Solution

    Given:

    [H+] = 1.33 × 10–3 M

    Molarity of acetic acid solution = 0.1 M

    Step 1: Calculation of Ka value of acetic acid

    Ka (acid dissociation constant) of acetic acid can be calculated using the below formula,

    Ka = [H+]^2/ [CH3COO-]

    Where [CH3COO-] is the concentration of acetate ion.

    Acetic acid dissociates as follows,

    CH3COOH + H2O ⇌ CH3COO- + H3O+

    From the balanced chemical equation, it is evident that the concentration of [CH3COO-] = [H3O+]


    Therefore, Ka = [H+]^2/ [CH3COO-] = [H+]^2/ [H+]

    Ka = [H+]

    Ka = 1.33 × 10–3 M


    Step 2: Calculation of pKa value of acetic acid

    pKa = -log(Ka)

    pKa = -log(1.33 × 10–3)

    pKa = 2.88


    Step 3: Calculation of pH of acetic acid solution

    pH of acetic acid solution can be calculated using the below formula,

    pH = pKa + log [salt]/[acid]


    Here, [salt] is the concentration of acetate ion and [acid] is the concentration of acetic acid.

    At equilibrium, the concentration of acetic acid and acetate ion is related by the Henderson-Hasselbalch equation,

    pH = pKa + log [salt]/[acid]

    pH = 2.88 + log [CH3COO-]/[CH3COOH]


    Substituting the values,

    pH = 2.88 + log (0.1/1.33 × 10–3)

    pH = 2.88 + 1.75

    pH = 4.63


    Answer:

    The pH of the 0.1 M acetic acid solution is 4.63, which is outside the given range of 2.86 to 2.89. Therefore, there might be an error in the given value of [H+].
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    The [H+] of 0.1 M acetic acid solution is 1.33 × 10–3. The pH of the solution (correct to two decimal places) is _______ .Correct answer is between `2.86,2.89`. Can you explain this answer?
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